Define the following and explain how they support either the wave or particle nature of light:
Wavelength –
Wavelength is the distance from the top of one wave to the top of the next. This requires light to be a wave
Frequency –
Frequency is the measure of how many waves go by in a second. This requires there to be waves to go by
Hertz –
Hertz is the unit of measure for frequency – 15 hertz means 15 waves per second. This requires waves
Photoelectric Effect –
The photoelectric effect is caused by light hitting metals and pushing electrons off atoms of the metal. In order for the electron to be pushed off, not simply moved to an excited state, it must be hit by something solid. This shows that light is also a particle.
Photon –
The photon is the particle of light with zero mass.
Write the formula that shows the relationship between frequency and wavelength. What is the relationship?
C=
λν, where c is the speed of light, λ is wavelength and ν is frequency
Wavelength and frequency are inversely proportional – one gets larger, the other gets smaller
Write the formula that shows the relationship between frequency and energy. What is the relationship?
E=hv, where E is energy, h is planck’s constant, and v is frequency
Energy and frequency are directly related – as frequency increases, energy increases
Combining the previous two, what is the relationship between wavelength and energy?
Wavelength and energy are inversely proportional – as wavelength gets larger, energy gets smaller
What segment of the visible spectrum has the most energy? The least?
Violet has the most energy, Red has the least energy
What segment of the electromagnetic spectrum has the most energy? The least?
Gamma rays have the most energy, radio waves have the least energy

Compare and contrast ground state and excited state.
In ground state, the electrons are in the lowest energy levels, while in excited state the electrons are in higher energy levels. This means that excited state electrons have more energy than ground state electrons.
How do quanta relate to an atom moving into an excited state?
A quantum is a specific amount of energy that an atom can absorb. This amount of energy is the exact amount of energy needed to move an electron from one orbital up to another orbital, thus creating an excited state. Atoms will have many quanta, as there are many higher orbitals that the electrons can be moved up into.
Explain the relationship between excited state and the color(s) emitted by an atom.
When an atom absorbs energy, it moves electrons to an excited state. When the electrons drop to lower energy levels, the atom releases energy in the form of light. The distance that the electron falls determines the amount of energy release, and thus the color of the light – a small fall = small energy = red light; a large fall = lots of energy = violet light.
Define line emission spectrum.
As electrons move up to excited states and then return, they release specific amounts of light.
These amounts give specific colors, so an atom will emit only colors corresponding to the energy released as electrons fall.
Contrast the energy of two atoms who have the following line emission spectrum:
Atom 1 – Red, Orange, and Green
Atom 2 – Orange, Green, and Blue
Atom 1 is absorbing and releasing less energy, as red has low energy and blue, emitted by atom 2, has more energy.
Explain the complete process of an atom eventually emitting both red and violet light, be sure to identify the original source of energy to make this possible.
To emit red light, an atom would need to absorb energy to move electrons to excited states, then the electron would need to fall a small distance to a lower orbital. To emit blue light, the electron would need to fall a greater distance to a lower orbital.
Give the names and letters for the four quantum numbers, then describe what each number is labeling.
N – principle quantum number = which energy level
L – angular momentum quantum number = which type of orbital
M - magnetic quantum number = which one of that orbital
Sp – spin of the electron = + ½ or – ½

In your own words, describe the following and explain what impact it has on the quantum numbers for electrons:
Aufbau Principle –
Orbitals of the least amount of energy are filled first, then the next amount of energy. This explains why we fill 4s before we fill 3d – 4s has less energy than 3d.
Pauli Exclusion Principle –
Each electron must have a unique set of quantum numbers. This means that two electrons that are in the same orbital of the same energy level must have opposite spins.
Hund’s Rule –
When electrons fill an orbital, like 3d, one electron of the same spin must be put into each orbital before a second electron is added to any orbital ( the “hate my brothers” rule for rooms in the house)
Write the electron configuration, the noble gas notation, and the orbital notation (using arrows) for the following elements. Circle three electrons shown in the orbital notation and give the quantum numbers for each.
Sulfur
1s 2 2s 2 2p 6 3s 2 3p 4
[Ne]3s 2 sp 4
1s↑↓2s↑↓2p↑↓ ↑ ↓ ↑↓3s ↑ ↓3p↑↓ ↑ ↑
2,1,0,-½
3,0,0,+½
Strontium
1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 5s 2
[Kr]5s 2
1s↑↓2s↑↓2p↑↓ ↑↓ ↑↓3s↑↓3p↑↓ ↑ ↑ 4s↑↓3d↑ ↓ ↑↓ ↑↓↑↓ ↑↓ 4p↑↓ ↑ ↓ ↑↓5s↑↓
3,2,-2,-½
4,1,0,+½
Cadmium
1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6 4d 10 5s 2
[Kr] 4d 10 5s 2
1s↑↓2s↑↓2p↑↓ ↑↓ ↑↓3s↑↓3p↑↓ ↑ ↑ 4s↑↓3d↑↓ ↑↓ ↑↓↑↓ ↑↓ 4p↑↓ ↑↓ ↑↓5s↑ ↓
4d↑↓ ↑↓ ↑↓↑↓ ↑ ↓
5,0,0,-½
4,2,2,-½

Write the electron configuration for the following elements, then determine the most likely ion to be formed:
Arsenic
1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 3
Arsenic is 3 electrons away from the octet (s 2 p 6 ), so it will gain 3 electrons, making it a -3 ion
Magnesium
1s 2 2s 2 2p 6 3s 2
Magnesium can reach the octet quicker by losing the 2 electrons in 3s 2 , than by gaining 6 electrons, so magnesium will lose the 2 electrons and form a -2 ion
Krypton
1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6
Krypton already has the octet, so it will not form any ions!!
What element is shown by the following electron configurations and noble gas notations?
1s 2 2s 2 2p 5
The element is in the 2 nd period, 5 th element in the P block, so it is Fluorine
1s 2 2s 2 2p 6 3s 2 sp 6 4s 2 3d 6
The element is in the 4 th period (due to 4s 2 ), and the 6 th element in the D block, so it is Iron
[Kr]5s 2 4d 4
The element is in the 5 th period (due to 5s 2 ), and the 4 th element in the D block, so it is Molybdenum
[Xe]6s 2 4f 8
The element is in the 6 th period (due to 6s 2 ), and the 8 th element in the F block, so it is Terbium